A. Use average bond energies together with the standard enthalpy of formation of C(g) (718.4 kJ/mol ) to estimate the standard e
nthalpy of formation of gaseous benzene, C6H6(g). (Remember that average bond energies apply to the gas phase only.)
B. Compare the value you obtain using average bond energies to the actual standard enthalpy of formation of gaseous benzene, 82.9 kJ/mol. What does the difference between these two values tell you about the stability of benzene?
B. Compare the value you obtain using average bond energies to the actual standard enthalpy of formation of gaseous benzene, 82.9 kJ/mol. What does the difference between these two values tell you about the stability of benzene?
1 answer:
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Answer : The final concentration of copper(II) ion is, 0.198 M
Explanation :
First we have to calculate the moles of and
.
Moles of = Moles of
= 0.00459 mol
and,
Moles of = Moles of
= 0.00869 mol
Now we have to calculate the total moles of copper(II) ion and total volume of solution.
Total moles copper(II) ion = 0.00459 mol + 0.00869 mol
Total moles copper(II) ion = 0.0133 mol
and,
Total volume of solution = 40.6 mL + 26.4 mL = 64.0 mL = 0.067 L (1 L = 1000 mL)
Now we have to calculate the final concentration of copper(II) ion.
Thus, the final concentration of copper(II) ion is, 0.198 M